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Published byAmber Henry Modified over 2 years ago

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The Reaction Quotient, Q Learning Goal: I will understand that the reaction quotient is the same as K, just not at equilibrium. I will understand how to compare the reaction quotient (Q) to the equilibrium constant (K) to determine it a system is at equilibrium, or what direction a shift will occur.

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What is Q? Q is a value we can use to determine if a reaction is at equilibrium. If a reaction is NOT at equilibrium, we can predict which direction (LEFT or RIGHT) the reaction will shift in order to reach equilibrium by comparing the value of Q to the value of K eq

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Comparing Q and K eq If Q

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How Do We Get the Value of Q? It is calculated exactly like K eq, EXCEPT the concentrations we plug in are NOT equilibrium concentrations. –They are just the concentrations of reactants and products at whatever time Q is calculated.

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Example #1: at 472 o C, K eq =.105 N 2 (g) + 3H 2 (g) 2NH 3 (g) 2 minutes after this reaction starts, you want to know if its at equilibrium so you measure the concentrations and find: a)What is the value of Q? b)In order to reach equilibrium, will this reaction shift left or right? [N 2 ] =.0020M [H 2 ] =.10M [NH 3 ] =.15M These are not necessarily Equilibrium concentrations

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Example # 1: Answer

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You Try # 1: K eq = 170 for CoCl 2 (g) Co(g) + Cl 2 (g) If [Co] = [Cl 2 ] =.15M and [CoCl 2 ] = 1.1x10 -3, is the reaction at equilibrium? If not, which way will it shift to reach equilibrium?

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You Try # 1: Answer

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How Did We Do? Learning Goal: I will understand that the reaction quotient is the same as K, just not at equilibrium. I will understand how to compare the reaction quotient (Q) to the equilibrium constant (K) to determine it a system is at equilibrium, or what direction a shift will occur.

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